Need help with item C only. Provided entire questions for FYI. Assume that coal

Question

Need help with item C only. Provided entire questions for FYI.

Assume that coal can be represented by the chemical formula C135H9609NS.

a. What is the percent of nitrogen by mass in coal? Answer = 0.73%

b. If 3 tons of coal is burned, what mass of nitrogen in the form of NO is produced? Assume that all of the nitrogen in the coal is converted to NO.

Mass of coal = 3 tons and formula for coal is C135H96O9NS. The reaction is written as C135H96O9NS + 156 O2 -----> 135 CO2 + 48 H2O + NO + SO2

Moles of 3 tons coal. Convert the given mass ton to g

1 ton = 907185 g

3 ton = 2.72*106 g

Moles of coal = 2.72*106 g / 1908.2730 g/mol =14253.7 moles

1 moles of C135H96O9NS = 1 moles of NO

14253.7 moles of C135H96O9NS = 14253.7 moles of NO

Mass of NO = 14253.7 moles * 30.06 g/mole

                     = 428467.7 g of NO

c. Actually more NO is produced than you just calculated. Explain.
Please help me explain why more NO was produced than calculated. Thanks.

Explanation / Answer

C) The Product of NO is more becuase ;

There during combustion the temperature is very high and at high temperature N2 present in air reacts with water and produce NO. Lets show the reaction

N2+ O2 ---> O2

So the amont of NO is more than it is calculated.

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